1. Limiting Reactants

2. When limited amounts of the reactants are mixed one reactant will run out before the other, limiting the amount of product that can be produced.
The reactant that runs out first is the limiting reactant.
The reactant that does not run out is the excess reactant.
The reaction can only produce as much product as the limiting reactant will produce.

3. C5H12 + 8O2 → 5CO2 + 6H2O
If g C5H12 reacts with g O2 according to the following equation, find (a) the limiting reactant, (b) the theoretical yield of CO2 (how much CO2 can be made) and (c) what mass of the excess reactant remains.

4. C5H12 + 8O2 → 5CO2 + 6H2O
If g C5H12 reacts with g O2 according to the following equation, find (a) the limiting reactant, (b) the theoretical yield of CO2 (how much CO2 can be made) and (c) what mass of the excess reactant remains.

5. 6Na + Fe2O3 → 3Na2O + 2Fe
If g Fe2O3 reacts with g Na according to the above equation, find (a) the limiting reactant, (b) the theoretical yield of Na2O (how much Na2O can be made) and (c) what mass of the excess reactant remains.

6. 6Na + Fe2O3 → 3Na2O + 2Fe
If g Fe2O3 reacts with g Na according to the above equation, find (a) the limiting reactant, (b) the theoretical yield of Na2O (how much Na2O can be made) and (c) what mass of the excess reactant remains.